1. The Cause of Chemical Change

2. Spontaneous Reactions:
A reaction is said to be spontaneous if, after being given the necessary energy to begin the reaction (activation energy), it occurs without continuous outside assistance
In other words, if reactants react then the reaction is spontaneous

3. Examples of spontaneous reactions
Melting ice
Spontaneous under right conditions

4. Dissolving sodium chloride
NaCl(s)  Na+(aq) + Cl-(aq)+ heat

5. Needs an initial spark to get started
Burning a candle
Needs an initial spark to get started

6. Spontaneous reactions can be very rapid or very slow
Silver tarnishing Cesium in water

7. Examples of non-spontaneous reactions
Decomposition of water – needs a continuous supply of energy or the reaction will stop

8. Building a brick wall
Needs the builder to keep working or the wall will stop being made

9. Non-spontaneous reactions occur at the expense of a previous spontaneous reaction
The reaction creating the electricity is spontaneous but the decomposition of water is not
The energy the brick layer is using is spontaneous but the building of the wall is not

10. Spontaneous reactions tend to be exothermic. (i. e
Spontaneous reactions tend to be exothermic. (i.e. they involve a loss in energy)
Products are more stable than reactants – this is why the reaction occurs

11. Why do endothermic reactions occur (i. e
Why do endothermic reactions occur (i.e. melting ice) if products are less stable than the reactants?

12. More than enthalpy change must be responsible for the spontaneity of a reaction  
Spontaneous reactions depend on :
Enthalpy
Entropy

13. Entropy (S) is a measure of the randomness or disorder of a system
Every chemical and physical change involves a change in the randomness or entropy of the system.

14. Throwing a new deck of cards in the air
Low entropy High entropy

15. Dissolving sodium chloride in water
Solid NaCl low entropy Aqueous NaCl high entropy

16. Spontaneous reactions and entropy
Spontaneous reactions tend to have an increase in entropy
i.e. Si < Sf OR ΔS > 0

17. Entropy increases when:
The volume of a gaseous system increases

18. 2) The temperature of a system increases

19. 3) The physical state of the system changes

20. 4) When the nproduct > nreactant
2NH3(g)  N2(g) + 3H2(g)

21. 5) A solid dissolves

22. 2NaHCO3(s)  Na2O(s) + H2O(l) + 2CO2(g)
6) solid reactants become liquid or gaseous products (or liquids become gases)
2NaHCO3(s)  Na2O(s) + H2O(l) + 2CO2(g)

23. Predict whether there is an increase in entropy (ΔS > 0) or a decrease in entropy (ΔS < 0):
1) steam condenses to water
2) solid CO2 sublimes
3) N2O4(g)  2NO2(g)
4) C3H8(g) + 5O2(g)  3CO2(g) + 4H2O(l)
5) H2(g) + ½ O2(g)  H2O(l)

24. Second Law of Thermodynamics:
All changes either directly or indirectly increase the entropy of the universe.

25. Third Law of Thermodynamics:
The entropy of a perfectly ordered crystal is zero at 0 K.

26. Standard Entropy So: the entropy change between 0 K and 298 K (i. e
Standard Entropy So: the entropy change between 0 K and 298 K (i.e.25oC)
H2O(l) H2O(g) O2(g) 1) All elements possess entropy 2) Units are in J/mol∙K 3) Entropy is temperature dependent (Enthalpy is not) 4) Unlike ΔHf , entropy values listed are not the change in entropy for a formation reaction but simply what the substance possesses

27. Standard Entropy Change: ΔSo
ΔSo = Σn SoP - Σn SoR
C3H8(g) + 5O2(g)  3CO2(g) + 4H2O(l)